Discussion Overview
The discussion revolves around the reactions of metal and non-metal oxides with water, specifically focusing on the formation of acids from non-metal oxides like sulfur trioxide. Participants explore the chemical equations involved and seek clarification on the underlying principles of these reactions.
Discussion Character
- Homework-related
- Technical explanation
- Debate/contested
Main Points Raised
- One participant expresses understanding of metallic oxides producing OH- ions in water but struggles with how non-metallic oxides, such as sulfur trioxide, form acids.
- Another participant confirms the first two equations presented by the original poster but points out an error in the charge balance of the last equation.
- A participant questions the dissociation of sulfuric acid into ions, suggesting a possible confusion over the charge of sulfate ions.
- There is curiosity about why only one oxygen atom from sulfur trioxide attaches to a hydrogen atom when it dissolves in water, rather than the other two.
- A participant emphasizes the importance of proper formatting in chemical equations and notes that sulfuric acid is the most stable form for energetic reasons, mentioning the existence of HSO4- and H3SO4+ in specific conditions.
- A question is raised about whether all non-metallic oxides must be polar molecules to form acids in water.
- Another participant challenges the classification of CO2 as a polar molecule.
Areas of Agreement / Disagreement
Participants generally agree on some aspects of the chemical equations but disagree on the details of charge balance and the nature of non-metallic oxides. The discussion remains unresolved regarding the properties of non-metallic oxides and their behavior in water.
Contextual Notes
There are unresolved questions about the dissociation of sulfuric acid and the characteristics of non-metallic oxides, including their polarity and how that relates to acid formation in water.